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Properties of small molecules

Edexcel IGCSE Chemistry

Topic questions Bonding, structure and the properties of matter Properties of small molecules

Properties of small molecules

19 questions · 204 marks · about 3.5 hours

Properties of small molecules questions

TopicProperties of small molecules

Chemistry Paper 1 June 2025, Question 5 14 marks

Also involves Intermolecular forces

Butane (C₄H₁₀) is an alkane.

(a)

Explain why butane is a saturated hydrocarbon.

[3]

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(b)

(b)(i)

When butane burns completely in oxygen, carbon dioxide and water are produced.

Give a chemical equation for this combustion reaction.

[2]

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(b)(ii)

Incomplete combustion can occur when the oxygen supply is limited.

One product of the incomplete combustion of butane is carbon monoxide.

Give the name of another product of this incomplete combustion.

[1]

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(b)(iii)

State why carbon monoxide is poisonous to humans.

[1]

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(c)

C₄H₁₀ exists as two isomers.

(c)(i)

State what is meant by the term isomers.

[2]

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(c)(ii)

Draw the displayed formula of each isomer.

[2]

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(d)

Explain why hexane (C₆H₁₄) has a higher boiling point than butane (C₄H₁₀).

[3]

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Chemistry Paper 1 November 2024, Question 2 6 marks

The table gives some information about five gases.

Name	Formula	Boiling point in °C
chlorine	Cl₂	–35
hydrogen chloride	HCl	–114
oxygen	O₂	–183
nitrogen	N₂	–196
hydrogen	H₂	–253

(a)

Use gases from the table to answer these questions.

You may use each gas once, more than once or not at all.

(a)(i)

Name the gas needed for combustion.

[1]

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(a)(ii)

Name the gas that is most abundant in air.

[1]

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(a)(iii)

Name the gas that can bleach damp litmus paper.

[1]

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(b)

Explain why hydrogen chloride is classified as a compound.

[2]

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(c)

Why does chlorine have the highest boiling point of the gases in the table?

$Question 2, shown as an image$

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Chemistry Paper 1 November 2024, Question 11 15 marks

Also involves Moles and amount of substance

This question is about the reactions of some compounds of lead.

(a)

Lead can be extracted from lead(II) sulfide, PbS, in two stages.

Stage 1 lead(II) sulfide is heated in air and reacts with oxygen to produce lead(II) oxide, PbO, and sulfur dioxide

Stage 2 lead(II) oxide is heated with carbon in a furnace

(a)(i)

Write a chemical equation for the reaction in stage 1.

[2]

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(a)(ii)

Give a reason why sulfur dioxide should not be released into the atmosphere.

[1]

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(a)(iii)

This is the equation for stage 2.

A mass of 892 tonnes of lead(II) oxide is heated in a furnace with an excess of carbon.

Calculate the maximum mass, in tonnes, of carbon dioxide that could be released into the atmosphere.

[1 tonne = 1 maths symbol 10⁶g]

[for PbO, M_r = 223 for CO₂, M_r = 44]

[3]

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(a)(iv)

The diagram shows the structures of lead(II) sulfide and sulfur dioxide.

Explain, in terms of bonding and structure, why lead(II) sulfide is a solid with a very high melting point at room temperature and why sulfur dioxide is a gas at room temperature.

lead(II) sulfide

[5]

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(b)

sulfur dioxide

A different oxide of lead contains 90.7% by mass of lead and 9.3% by mass of oxygen.

Determine the empirical formula of this oxide of lead.

[4]

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Chemistry Paper 1 June 2024 (R), Question 9 14 marks

(a)

The table shows the formulae of some positive and negative ions, and the formulae of some compounds containing these ions.

	Cl⁻	O²⁻	SO₄²⁻
Na⁺		Na₂O	Na₂SO₄
NH₄⁺	NH₄Cl
Zn²⁺	ZnCl₂		ZnSO₄

(a)(i)

Complete the table by giving the formulae of the missing compounds.

[3]

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(a)(ii)

Give the name of the compound with the formula ZnSO₄

[1]

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(b)

Hydrogen chloride and magnesium chloride have different types of bonding and have different structures.

(b)(i)

Complete the dot-and-cross diagram to show the outer shell electrons in a molecule of hydrogen chloride.

H C l

[2]

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(b)(ii)

The diagram shows the electronic configuration of a magnesium atom and of a chlorine atom.

Draw the electronic configuration of a magnesium ion and of a chloride ion in the boxes.

Show the charge on each ion.

[3]

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(b)(iii)

Explain why magnesium chloride has a much higher melting point than hydrogen chloride.

Refer to structure and bonding in your answer.

[5]

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Chemistry Paper 1 November 2023, Question 3 12 marks

Also involves Intermolecular forces

Crude oil is an important source of organic compounds.

(a)

The diagram shows how crude oil can be separated into useful mixtures of hydrocarbons.

(a)(i)

Give the name of this method of separation.

[1]

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(a)(ii)

State what happens to the crude oil when it is in X.

[1]

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(a)(iii)

Give the letter of the mixture that is most likely to contain a hydrocarbon with six carbon atoms.

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(a)(iv)

Give the name of mixture D.

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(a)(v)

Give a use for mixture B.

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(b)

Explain, in terms of intermolecular forces, why a hydrocarbon in mixture B has a higher boiling point than a hydrocarbon in mixture D.

[3]

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(c)

Catalytic cracking can be used to break down long‑chain hydrocarbons to produce shorter‑chain alkanes and alkenes.

(c)(i)

Give the name of a catalyst used in catalytic cracking.

[1]

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(c)(ii)

Complete the equation to show two different alkenes that could be produced in this cracking reaction.

$Question 3, shown as an image$

[2]

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(c)(iii)

Give one important use for short‑chain alkenes.

[1]

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Chemistry Paper 1 June 2023, Question 3 6 marks

Also involves Bonding, structure and the properties of matter

The table gives some information about three substances, X, Y and Z.

(a)

Complete the table by giving the missing information.

[4]

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(b)

Explain why substance X has a low melting point.

[2]

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Chemistry Paper 1 June 2023 (R), Question 10 15 marks

Also involves Alcohols · Intermolecular forces

This question is about propene.

(a)(i)

The structural formula of propene is CH₃CH $fraction$ CH₂

Complete the dot-and-cross diagram for a molecule of propene.

[2]

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(a)(ii)

Describe the forces of attraction that hold the atoms together in a molecule of propene.

[2]

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(b)

The alkane pentadecane has the formula C₁₅H₃₂

Describe how propene can be produced from pentadecane.

[2]

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(c)

Propene is used to make poly(propene).

(c)(i)

Complete the equation for the formation of poly(propene).

$Question 10, shown as an image$

[2]

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(c)(ii)

Explain why the disposal of poly(propene) in landfill sites is a problem.

[2]

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(d)

Propene can be converted into compound X.

(d)(i)

Compound X contains these percentages by mass.

• carbon 60%

• hydrogen 13.3%

• oxygen 26.7%

Compound X has an M_r of 60

Determine the molecular formula of compound X.

[3]

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(d)(ii)

Propene and compound X both have simple molecular structures.

Explain why compound X has a higher boiling point than propene.

[2]

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Chemistry Paper 1 January 2023 (R), Question 8 12 marks

This question is about the oxides of some elements in Group 4 of the Periodic Table.

(a)

When 5.34 g of lead(II) carbonate are heated, lead(II) oxide and carbon dioxide are formed.

This is the equation for the reaction.

$Question 8, shown as an image$

(a)(i)

Give the name for this type of reaction.

[1]

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(a)(ii)

Calculate the maximum mass of lead(II) oxide that can be formed from 5.34 g of lead(II) carbonate.

[for PbCO₃, M_r = 267 for PbO, M_r = 223]

[2]

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(b)

The diagram shows apparatus used to heat lead(II) carbonate.

(b)(i)

Complete the diagram to show what needs to be added to the apparatus to test that the gas released is carbon dioxide.

[2]

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(b)(ii)

Give the result of the test.

[1]

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(c)

Silicon dioxide (SiO₂) and carbon dioxide both contain covalent bonds.

Silicon dioxide is a solid with a high melting point. Carbon dioxide is a gas at room temperature.

Explain why silicon dioxide has a much higher melting point than carbon dioxide.

Refer to structure and bonding in your answer.

[6]

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Chemistry Paper 1 January 2023, Question 9 10 marks

This question is about substances that contain covalent bonds.

(a)

The diagram represents a molecule of oxygen.

Describe the forces of attraction in a covalent bond.

[2]

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(b)

The table shows the boiling points of three Group 7 elements.

	Boiling point in °C
fluorine	–188
chlorine	–34
bromine	59

Explain the trend in the boiling points.

[3]

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(c)

Graphite is a naturally-occurring form of carbon.

Explain why graphite is soft and conducts electricity.

Refer to structure and bonding in your answer.

[5]

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Chemistry Paper 1 June 2022 (R), Question 6 9 marks

Silicon hydride (SiH₄) and silicon dioxide (SiO₂) both contain covalent bonds but they have different structures.

(a)

Describe the forces of attraction in a covalent bond.

[2]

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(b)

Complete the diagram to show the outer shell electrons in a molecule of silicon hydride (SiH₄).

[1]

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(c)

The diagram represents part of the structure of silicon dioxide (SiO₂).

(c)(i)

State how the diagram shows that the atom labelled A is oxygen, not silicon.

[1]

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(c)(ii)

Silicon hydride has a simple molecular structure.

Silicon dioxide has the same type of structure as diamond.

Explain why silicon dioxide has a much higher melting point than silicon hydride.

Refer to structure and bonding in your answer.

[4]

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(d)

Silicon hydride reacts with oxygen to form silicon dioxide and water.

Write a chemical equation for the reaction between silicon hydride and oxygen.

[1]

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Chemistry Paper 1 June 2022, Question 8 10 marks

Diamond and graphite are giant covalent structures made of carbon atoms.

The diagram shows their structures.

(a)

Discuss the differences between diamond and graphite.

Refer to structure and bonding, electrical conductivity and hardness in your answer.

[6]

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(b)

C₆₀ fullerene is a simple molecular substance made of 60 carbon atoms.

The diagram shows its structure.

The table shows the approximate melting points of diamond, graphite and C₆₀ fullerene.

Substance	Approximate melting point in °C
diamond	4000
graphite	3600
C₆₀ fullerene	600

Explain why C₆₀ fullerene has a much lower melting point than diamond and graphite.

[4]

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Chemistry Paper 1 June 2022 (R), Question 10 10 marks

Also involves Chemical measurements and uncertainty

A student investigates how the electrical conductivity changes as dilute sulfuric acid is added to barium hydroxide solution.

This is the student’s method.

Step 1 =$~dd=RMKM cm³ of barium hydroxide solution to a beaker

Step 2 maths symbol measure the electrical conductivity of the solution

Step 3 =$~dd=NMKM cm³ of dilute sulfuric acid to the beaker

Step 4 maths symbol stir the mixture

Step 5 maths symbol measure the electrical conductivity of the mixture

Step 6 maths symbol repeat steps 3 to 5 until a total of 100 cm3³ of dilute sulfuric acid has been added

The table shows the student’s results.

Total volume of acid added in cm³	Electrical conductivity in arbitrary units
0.0	10.0
10.0	8.0
20.0	7.2
30.0	4.0
40.0	2.0
50.0	0.0
60.0	1.4
70.0	2.8
80.0	4.2
90.0	5.6
100.0	7.0

(a)(i)

Name a piece of apparatus the student could use to add 10.0 cm³ of dilute sulfuric acid to the beaker.

[1]

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(a)(ii)

Plot the student’s results.

[2]

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(a)(iii)

Ignoring the anomalous result, draw two lines of best fit, making sure that the two lines cross.

Total volume of acid added in cm³

[1]

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(a)(iv)

Give the trend shown on the graph for the first 50 cm³ of acid added.

[1]

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(a)(v)

Suggest a mistake the student could have made to cause the anomalous result.

[1]

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(b)

This is the equation for the reaction.

$Question 10, shown as an image$

(b)(i)

When 50 cm³ of dilute sulfuric acid have been added, only barium sulfate and water are present in the mixture.

Explain why this mixture does not conduct electricity. Refer to the type of bonding in barium sulfate and in water in your answer.

[3]

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(b)(ii)

Name a technique the student could use to separate barium sulfate from the mixture after 100 cm³ of dilute sulfuric acid has been added.

[1]

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Chemistry Paper 1 January 2022, Question 10 9 marks

This question is about substances with covalent bonds.

(a)(i)

Draw a dot and cross diagram to show the outer shell electrons in a molecule

$Question 10, shown as an image$

[2]

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(a)(ii)

Describe the forces of attraction in a covalent bond.

[2]

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(b)

The diagram shows three different structures of carbon.

(b)(i)

Name structure A.

[1]

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(b)(ii)

Graphite and C₆₀ fullerene contain covalent bonds, but have different structures.

Explain why C₆₀ fullerene has a much lower melting point than graphite.

Refer to structure and bonding in your answer.

[4]

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Chemistry Paper 1 January 2021 (R), Question 7 8 marks

The formation of ions and covalent bonds involves electrons.

The table gives the electronic configurations of atoms of hydrogen, lithium and chlorine.

Element	Electronic configuration of atom
hydrogen	1
lithium	2.1
chlorine	2.8.7

(a)

Describe the different roles of electrons in the formation of

maths symbol ions in lithium chloride

maths symbol covalent bonds in hydrogen chloride

[3]

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(b)

Explain why lithium chloride has a higher melting point than hydrogen chloride.

Refer to structure and bonding in your answer.

[5]

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Chemistry Paper 1 November 2020, Question 5 12 marks

(a)

Chlorine, bromine and iodine are elements in the Periodic Table.

Explain how the position of these elements in the Periodic Table depends on their electronic configurations.

[2]

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(b)

Chlorine reacts with methane to form CH₃Cl and HCl

(b)(i)

State the condition necessary for this reaction.

[1]

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(b)(ii)

Give the equation for this reaction.

[1]

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(b)(iii)

The bonds in a molecule of CH₃Cl are covalent.

Explain, in terms of electrostatic attractions, what is meant by a covalent bond.

[2]

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(b)(iv)

[2]

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(b)(v)

CH₃Cl has a simple molecular structure.

Explain why CH₃Cl has a low boiling point.

[2]

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(c)

Graphite is another substance that contains covalent bonds.

The diagram shows the structure of graphite.

Most covalent substances do not conduct electricity.

Explain why graphite is able to conduct electricity.

[2]

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Chemistry Paper 1 November 2020 (R), Question 9 11 marks

This question is about some compounds of the elements in Group 4 of the Periodic Table.

(a)

When carbon dioxide dissolves in water, a weak acid forms.

(a)(i)

Which of these could be the pH of this weak acid?

$Question 9, shown as an image$

[1]

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(a)(ii)

Which of these is a correct statement about acids?

$Question 9, shown as an image$

[1]

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(b)

When lead(II) carbonate is heated, lead(II) oxide and carbon dioxide form.

(b)(i)

Give the name of this type of reaction.

[1]

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(b)(ii)

Complete the equation for this reaction.

[1]

(c)

Silicon dioxide, SiO₂, and silicon(IV) chloride, SiCl₄, are both covalently bonded compounds.

The table shows the melting and boiling points of these two compounds, and the physical state of silicon dioxide at room temperature.

Compound	Melting point in °C	Boiling point in °C	Physical state at room temperature
SiO₂	1710	2230	solid
SiCl₄	−69	58

(c)(i)

Complete the table by giving the physical state of silicon(IV) chloride at room temperature.

[1]

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(c)(ii)

Explain, in terms of structure and bonding, why silicon dioxide has a much higher melting point than silicon(IV) chloride.

[6]

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Chemistry Paper 1 January 2020, Question 8 11 marks

(a)

Carbon dioxide changes directly from a solid to a gas without becoming a liquid.

(a)(i)

Give the name of the change of state from solid to gas.

[1]

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(a)(ii)

Describe the test for carbon dioxide gas.

[2]

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(b)

Carbon dioxide is a simple molecular covalent substance.

Explain why carbon dioxide turns from a solid to a gas at a very low temperature.

[2]

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(c)

Diamond and graphite are both giant covalent substances made up of carbon atoms.

● diamonds are used in cutting tools

● graphite is used in pencils to make marks on paper

Explain, with reference to structure and bonding, why each substance is suitable for its particular use.

[6]

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Chemistry Paper 1 January 2020 (R), Question 10 11 marks

This question is about carbon and its compounds.

(a)(i)

Draw a dot-and-cross diagram to show the outer shell electrons in a molecule

$Question 10, shown as an image$

[2]

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(a)(ii)

The atoms in carbon dioxide are held together by covalent bonds.

Describe the forces of attraction in a covalent bond.

[2]

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(b)

The diagram shows three different structures of carbon.

(b)(i)

Explain why graphite conducts electricity.

[2]

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(b)(ii)

Explain why diamond has a much higher melting point than C₆₀ fullerene.

Refer to structure and bonding in your answer.

[5]

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Chemistry Paper 2 June 2019, Question 3 9 marks

Also involves Chemical measurements and uncertainty · Alcohols · Hazard symbols and risk assessment · Intermolecular forces

Methanol, ethanol, propanol and butanol are alcohols. They are all liquids that evaporate easily when warmed.

A student uses this apparatus to compare the time taken for the four liquids to evaporate.

She uses this method.

• pour some methanol into an evaporating basin

• place the evaporating basin on top of a beaker containing hot water

• measure the time taken for the methanol to evaporate completely

• repeat the experiment with each of the other alcohols, using the same apparatus

(a)

State two variables the student should control to make sure her results are valid.

[2]

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(b)

State why it is not safe to heat the evaporating basin directly with a Bunsen flame.

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(c)

The table shows the results of experiments done by four students, A, B, C and D.

	Formula			Time taken for liquid to evaporate in s
Alcohol	of alcohol	Student A	Student B	Student C	Student D	Mean time in s
methanol	CH₃OH	20	24	22	26	23
ethanol	C₂H₅OH	32	34	35	30	33
propanol	C₃H₇OH	45	47	50	48	48
butanol	C₄H₉OH	64	63	90	60

(c)(i)

Calculate the mean (average) time for butanol to evaporate.

[2]

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(c)(ii)

Explain how the results show which alcohol evaporates most easily.

[2]

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(c)(iii)

State the relationship between the number of carbon atoms in the molecule and how easily the alcohol evaporates.

[2]

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Chemistry Paper 1 June 2025, Question 5 Chemistry Paper 1 · June 2025 · Question 5 14 marks

Chemistry Paper 1 November 2024, Question 2 Chemistry Paper 1 · November 2024 · Question 2 6 marks

Chemistry Paper 1 November 2024, Question 11 Chemistry Paper 1 · November 2024 · Question 11 15 marks

Chemistry Paper 1 June 2024 (R), Question 9 Chemistry Paper 1 · June 2024 (R) · Question 9 14 marks

Chemistry Paper 1 November 2023, Question 3 Chemistry Paper 1 · November 2023 · Question 3 12 marks

Chemistry Paper 1 June 2023, Question 3 Chemistry Paper 1 · June 2023 · Question 3 6 marks

Chemistry Paper 1 June 2023 (R), Question 10 Chemistry Paper 1 · June 2023 (R) · Question 10 15 marks

Chemistry Paper 1 January 2023 (R), Question 8 Chemistry Paper 1 · January 2023 (R) · Question 8 12 marks

Chemistry Paper 1 January 2023, Question 9 Chemistry Paper 1 · January 2023 · Question 9 10 marks

Chemistry Paper 1 June 2022 (R), Question 6 Chemistry Paper 1 · June 2022 (R) · Question 6 9 marks

Chemistry Paper 1 June 2022, Question 8 Chemistry Paper 1 · June 2022 · Question 8 10 marks

Chemistry Paper 1 June 2022 (R), Question 10 Chemistry Paper 1 · June 2022 (R) · Question 10 10 marks

Chemistry Paper 1 January 2022, Question 10 Chemistry Paper 1 · January 2022 · Question 10 9 marks

Chemistry Paper 1 January 2021 (R), Question 7 Chemistry Paper 1 · January 2021 (R) · Question 7 8 marks

Chemistry Paper 1 November 2020, Question 5 Chemistry Paper 1 · November 2020 · Question 5 12 marks

Chemistry Paper 1 November 2020 (R), Question 9 Chemistry Paper 1 · November 2020 (R) · Question 9 11 marks

Chemistry Paper 1 January 2020, Question 8 Chemistry Paper 1 · January 2020 · Question 8 11 marks

Chemistry Paper 1 January 2020 (R), Question 10 Chemistry Paper 1 · January 2020 (R) · Question 10 11 marks

Chemistry Paper 2 June 2019, Question 3 Chemistry Paper 2 · June 2019 · Question 3 9 marks

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Chemistry Paper 1 November 2024, Question 2 6 marks

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Chemistry Paper 1 June 2024 (R), Question 9 14 marks

Chemistry Paper 1 November 2023, Question 3 12 marks

Chemistry Paper 1 June 2023, Question 3 6 marks

Chemistry Paper 1 June 2023 (R), Question 10 15 marks

Chemistry Paper 1 January 2023 (R), Question 8 12 marks

Chemistry Paper 1 January 2023, Question 9 10 marks

Chemistry Paper 1 June 2022 (R), Question 6 9 marks

Chemistry Paper 1 June 2022, Question 8 10 marks

Chemistry Paper 1 June 2022 (R), Question 10 10 marks

Chemistry Paper 1 January 2022, Question 10 9 marks

Chemistry Paper 1 January 2021 (R), Question 7 8 marks

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